merits and demerits of bohr atom model
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Niels Bohr proposed the Bohr Model of the Atom in 1915. Because the Bohr Model is a modification of the earlier Rutherford Model, some people call Bohr's Model the Rutherford-Bohr Model. The modern model of the atom is based on quantum mechanics. The Bohr Model contains some errors, but it is important because it describes most of the accepted features of atomic theory without all of the high-level math of the modern version. Unlike earlier models, the Bohr Model explains the Rydberg formula for the spectral emission lines of atomic hydrogen.
The Bohr Model is a planetary model in which the negatively-charged electrons orbit a small, positively-charged nucleus similar to the planets orbiting the Sun (except that the orbits are not planar). The gravitational force of the solar system is mathematically akin to the Coulomb (electrical) force between the positively-charged nucleus and the negatively-charged electrons.
Main Points of the Bohr Model
Electrons orbit the nucleus in orbits that have a set size and energy.
The energy of the orbit is related to its size. The lowest energy is found in the smallest orbit.
Radiation is absorbed or emitted when an electron moves from one orbit to another.
Bohr Model of Hydrogen
The simplest example of the Bohr Model is for the hydrogen atom (Z = 1) or for a hydrogen-like ion (Z > 1), in which a negatively-charged electron orbits a small positively-charged nucleus. Electromagnetic energy will be absorbed or emitted if an electron moves from one orbit to another. Only certain electron orbits are permitted. The radius of the possible orbits increases as n2, where n is the principal quantum number. The 3 → 2 transition produces the first line of the Balmer series. For hydrogen (Z = 1) this produces a photon having wavelength 656 nm (red light).
Problems with the Bohr Model
It violates the Heisenberg Uncertainty Principle because it considers electrons to have both a known radius and orbit.
The Bohr Model provides an incorrect value for the ground state orbital angular momentum.
It makes poor predictions regarding the spectra of larger atoms.
It does not predict the relative intensities of spectral lines.
The Bohr Model does not explain fine structure and hyperfine structure in spectral lines.
It does not explain the Zeeman Effect. Hope this helps!
The Bohr Model is a planetary model in which the negatively-charged electrons orbit a small, positively-charged nucleus similar to the planets orbiting the Sun (except that the orbits are not planar). The gravitational force of the solar system is mathematically akin to the Coulomb (electrical) force between the positively-charged nucleus and the negatively-charged electrons.
Main Points of the Bohr Model
Electrons orbit the nucleus in orbits that have a set size and energy.
The energy of the orbit is related to its size. The lowest energy is found in the smallest orbit.
Radiation is absorbed or emitted when an electron moves from one orbit to another.
Bohr Model of Hydrogen
The simplest example of the Bohr Model is for the hydrogen atom (Z = 1) or for a hydrogen-like ion (Z > 1), in which a negatively-charged electron orbits a small positively-charged nucleus. Electromagnetic energy will be absorbed or emitted if an electron moves from one orbit to another. Only certain electron orbits are permitted. The radius of the possible orbits increases as n2, where n is the principal quantum number. The 3 → 2 transition produces the first line of the Balmer series. For hydrogen (Z = 1) this produces a photon having wavelength 656 nm (red light).
Problems with the Bohr Model
It violates the Heisenberg Uncertainty Principle because it considers electrons to have both a known radius and orbit.
The Bohr Model provides an incorrect value for the ground state orbital angular momentum.
It makes poor predictions regarding the spectra of larger atoms.
It does not predict the relative intensities of spectral lines.
The Bohr Model does not explain fine structure and hyperfine structure in spectral lines.
It does not explain the Zeeman Effect. Hope this helps!
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Bohr's atomic model
Merits:
1) Bohr's atomic model explained the stability of an atom. According to Bohr, an electron revolving in a particular orbit cannot lose energy. Therefore, emission of radiation is not possible as long as the electron remains in one of its energy levels and hence there is no cause of insatbility in his model.
2) Bohr's concept of atom explained successfully the atomic spectra of hydrogen atom. From the Bohr's atomic model, it is clear that electron can have only certain definite energy levels. When the electron is present as close to the nucleus as possible, the atom has the minimum possible energy and is said to be in the ground state. When energy from some outside source is supplied to it, it can absorb a definite amount of energy and jumps to higher energy state. Such state of an atom possesses more energy than possessed in the ground state is called the excited state.
3) Bohr's theory could predict the values of energies which an electron can have while revolving around the nucleus of hydrogen in hydrogen atom.
Demrits:
1) Bohr's model of an atom could not account for the finer details of the hydrogen spectrum observed using sophisticated spectroscopic techniques.
2) It could not explain line spectra of atoms containing more than one electron called multielectron atoms.
3) it failed to account for the effect of magnetic field on the spectra of atoms or ions, that is splitting of spectral lines further in presence of magnetic field called as Zeeman effect.
4) Similarly it could explain the effect of electric field on the spectra of atoms (known as Stark effect)
5) It could not provide clue to explain the shapes of molecules arising out of the directional bonding between atoms.
hopefully this helped uh !
mark it as brainliest ..
here is ur answer ...
Bohr's atomic model
Merits:
1) Bohr's atomic model explained the stability of an atom. According to Bohr, an electron revolving in a particular orbit cannot lose energy. Therefore, emission of radiation is not possible as long as the electron remains in one of its energy levels and hence there is no cause of insatbility in his model.
2) Bohr's concept of atom explained successfully the atomic spectra of hydrogen atom. From the Bohr's atomic model, it is clear that electron can have only certain definite energy levels. When the electron is present as close to the nucleus as possible, the atom has the minimum possible energy and is said to be in the ground state. When energy from some outside source is supplied to it, it can absorb a definite amount of energy and jumps to higher energy state. Such state of an atom possesses more energy than possessed in the ground state is called the excited state.
3) Bohr's theory could predict the values of energies which an electron can have while revolving around the nucleus of hydrogen in hydrogen atom.
Demrits:
1) Bohr's model of an atom could not account for the finer details of the hydrogen spectrum observed using sophisticated spectroscopic techniques.
2) It could not explain line spectra of atoms containing more than one electron called multielectron atoms.
3) it failed to account for the effect of magnetic field on the spectra of atoms or ions, that is splitting of spectral lines further in presence of magnetic field called as Zeeman effect.
4) Similarly it could explain the effect of electric field on the spectra of atoms (known as Stark effect)
5) It could not provide clue to explain the shapes of molecules arising out of the directional bonding between atoms.
hopefully this helped uh !
mark it as brainliest ..
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